A-level Chemistry Question paper Paper 1 June 2018 - CIE Notes

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A-level

CHEMISTRY

Paper 1 Inorganic and Physical Chemistry

Tuesday 5 June 2018

Afternoon

Time allowed: 2 hours

Materials

For this paper you must have:

? the Periodic Table/Data Booklet, provided as an insert (enclosed)

? a ruler with millimetre measurements

? a scientific calculator, which you are expected to use where appropriate.

For Examiner¡¯s Use

Question

Mark

1

2

3

Instructions

Use black ink or black ball-point pen.

Fill in the boxes at the top of the page.

Answer all questions.

You must answer the questions in the spaces provided. Do not write outside

the box around each page or on blank pages.

? All working must be shown.

? Do all rough work in this book. Cross through any work you do not want to be

marked.

?

?

?

?

Information

4

5

6

7

8

9

10

TOTAL

? The marks for questions are shown in brackets.

? The maximum mark for this paper is 105.

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Answer all questions in the spaces provided.

0 1

This question is about lattice enthalpies.

0 1 . 1

Figure 1 shows a Born¨CHaber cycle for the formation of magnesium oxide.

Complete Figure 1 by writing the missing symbols on the appropriate energy levels.

[3 marks]

Figure 1

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0 1 . 2

Table 1 contains some thermodynamic data.

Table 1

Enthalpy change

/ kJ mol¨C1

Enthalpy of formation for magnesium oxide

¨C602

Enthalpy of atomisation for magnesium

+150

First ionisation energy for magnesium

+736

Second ionisation energy for magnesium

+1450

Bond dissociation enthalpy for oxygen

+496

First electron affinity for oxygen

¨C142

Second electron affinity for oxygen

+844

Calculate a value for the enthalpy of lattice formation for magnesium oxide.

Enthalpy of lattice formation

[3 marks]

kJ mol¨C1

Turn over for the next question

Turn over ?

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0 2

0 2 . 1

Nitrogen and hydrogen were mixed in a 1:3 mole ratio and left to reach equilibrium in

a flask at a temperature of 550 K. The equation for the reaction between nitrogen and

hydrogen is shown.

N2(g) + 3H2(g) ? 2NH3(g)

When equilibrium was reached, the total pressure in the flask was 150 kPa and the

mole fraction of NH3(g) in the mixture was 0.80

Calculate the partial pressure of each gas in this equilibrium mixture.

0 2 . 2

[3 marks]

Partial pressure of nitrogen

kPa

Partial pressure of hydrogen

kPa

Partial pressure of ammonia

kPa

Give an expression for the equilibrium constant (Kp) for this reaction.

[1 mark]

Kp

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0 2 . 3

In a different equilibrium mixture, under different conditions, the partial pressures of

the gases are shown in Table 2.

Table 2

Gas

Partial pressure / kPa

N2

1.20 ¡Á 102

H2

1.50 ¡Á 102

NH3

1.10 ¡Á 103

Calculate the value of the equilibrium constant (Kp) for this reaction and give its units.

[2 marks]

Kp

0 2 . 4

Units

The enthalpy change for the reaction is ¨C92 kJ mol¨C1

State the effect, if any, of an increase in temperature on the value of Kp for this

reaction.

Justify your answer.

[3 marks]

Effect on Kp

Justification

9

Turn over ?

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